Calculate Gibbs energy change for a reaction having $\Delta \mathrm{H}=31400 \mathrm{~J}, \Delta \mathrm{~S}=32 \mathrm{JK}^{-1}$ at $1000^{\circ} \mathrm{C}$ ?

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Aicharya · Accepted Answer

$\begin{aligned} & \mathrm{T}=1000^{\circ} \mathrm{C}=1273 \mathrm{~K} \ & \Delta \dot{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{~S} \ & =31400 \mathrm{~J}-1273 \mathrm{~K}\left(32 \mathrm{~J} \mathrm{~K}^{-1}ight) \ & =3.1400 \mathrm{~J}-40736 \mathrm{~J} \ & \Delta \mathrm{G}=-9336 \mathrm{~J} \end{aligned}$

Calculate Gibbs energy change for a reaction having $\Delta \mathrm{H}=31400 \mathrm{~J}, \Delta…

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